Electrochemical cell

ABSTRACT

An electrochemical cell comprises as an anode, a lithium transition metal oxide or sulphide compound which has a [B 2 ]X 4   n−  spinel-type framework structure of an A[B 2 ]X 4  spinel wherein A and B are metal cations selected from Li, Ti, V, Mn, Fe and Co, X is oxygen or sulphur, and n− refers to the overall charge of the structural unit [B 2 ]X 4  of the framework structure. The transition metal cation in the fully discharged state has a mean oxidation state greater than +3 for Ti, +3 for V, +3.5 for Mn, +2 for Fe and +2 for Co. The cell includes as a cathode, a lithium metal oxide or sulphide compound. An electrically insulative lithium containing liquid or polymeric electronically conductive electrolyte is provided between the anode and the cathode.

THIS INVENTION relates to an electrochemical cell.

This application is continuation of U.S. application Ser. No. 12/823,977filed Jun. 25, 2010, now U.S. Pat. No. 7,855,016, which is acontinuation of U.S. application Ser. No. 11/931,490 filed Oct. 31,2007, now U.S. Pat. No. 7,824,804, which is a divisional of U.S.application Ser. No. 10/228,734 filed Aug. 27, 2002, now U.S. Pat. No.7,452,630, which is a continuation of U.S. application Ser. No.08/206,792 filed Mar. 4, 1994, abandoned, which claims priority to SouthAfrican Application No. 93/6488 filed Sep. 2, 1993. The entire text ofeach of the above-referenced disclosures is specifically incorporatedherein by reference without disclaimer.

According to the invention, there is provided an electrochemical cell,which comprises

-   -   as at least part of an anode, a lithium transition metal oxide        or sulphide compound which has a [B₂]X₄ ^(n−) spinel-type        framework structure of an A[B₂]X₄ spinel wherein A and B are        metal cations selected from Li, Ti, V, Mn, Fe and Co, X is        oxygen (O) or sulphur (S), and n− refers to the overall charge        of the structural unit [B₂]X₄ of the framework structure, and        the transition metal cation of which in its fully discharged        state has a mean oxidation state greater than +3 for Ti, +3 for        V, +3.5 for Mn, +2 for Fe and +2 for Co;    -   as at least part of a cathode, a lithium metal oxide or sulphide        compound; and    -   an electrically insulative lithium containing liquid or        polymeric electronically conductive electrolyte between the        anode and the cathode, such that, on discharging the cell,        lithium ions are extracted from the spinel-type framework        structure of the anode, with the oxidation state of the metal        ions of the anode thereby increasing, while a concomitant        insertion of lithium ions into the compound of the cathode takes        place, with the oxidation state of the metal ions of the cathode        decreasing correspondingly.

The compounds of the anode and cathode may, in particular, be lithiummetal oxide compounds.

While the cell can be a primary cell, it is envisaged that it may, inparticular, be a rechargeable or secondary cell in which the reversereactions to those set out above, take place during charging of thecell.

Thus, spinel compounds have structures that can be represented by thegeneral formula A[B₂]X₄ given hereinbefore, and in which the X atoms areideally arranged in a cubic-close-packed fashion to form a negativelycharged anion array comprised of face-sharing and edge-sharing Xtetrahedra and octahedra. In the formula A[B₂]X₄, the A cations and Bcations occupy tetrahedral and octahedral sites respectively. In theideal spinel structure, with the origin of the unit cell at the centre (3m), the close-packed anions are located at the 32e positions of thespace group Fd3m. Each unit cell contains 64 tetrahedral intersticessituated at three crystallographically non-equivalent positions 8a, 8band 48f, and 32 octahedral interstices situated at thecrystallographically non-equivalent positions 16c and 16d.

In the A[B₂]X₄ spinel, the A cations reside in the 8a tetrahedralinterstices and the B cations in the 16d octahedral interstices. Thereare thus 56 empty tetrahedral and 16 empty octahedral sites per cubicunit cell.

The framework structure of the lithium metal oxide compound of the anodethus has, as its basic structural unit, a unit of the formula [B₂]X₄^(n−) as hereinbefore described.

In the anode of the cell of the present invention, therefore, the Bcations of the [B₂]X₄ ^(n−) host framework structure may be regarded asbeing located at the 16d octahedral positions, and the X anions as beinglocated at the 32e positions of the spinel structure. The tetrahedradefined by the 8a, 8b and 48f positions and the octahedra defined by the16c positions of the spinel structure thus form, the interstitial spaceof the [B₂]X₄ ^(n−) framework structure for the diffusion of mobile Li⁺cations.

The B cations of the framework structure may consist of one cationictype, or more than one cationic type of identical or mixed valence toprovide various [B₂]X₄ ^(n−) framework structures, the overall charge ofwhich can vary over a wide range.

Spinel compounds having the [B₂]X₄ ^(n−) framework structure may also becharacterized by crystallographic space groups other than the prototypiccubic space group Fd3m, and may therefore not have the idealcubic-close-packed structures hereinbefore described. For example, inLi_(1+x)[Mn₂]O₄ compounds with 0≦x≦1, ie compounds in which A is Li, andB is Mn, the spinel structure is distorted, as a result of theJahn-Teller Mn³⁺ octahedral site ions, to tetragonal symmetry, and thecompound is characterized by the tetragonal space groups F4₁/ddm, or,alternatively, I4₁/amd in which the tetrahedral and octahedral sitenomenclature differs from that as defined by the space group Fd3m.

Furthermore, the anode need not necessarily be a stoichiometric spinelcompound, but can instead be a defect spinel. Defect spinels are wellknown in the large family of spinel compounds and can have vacancies onthe A sites, or on the B sites, or on both the A sites and B sites. Forexample, compounds can be synthesized in which defects are created byvarying the quantity of B cations in the framework structure such thatadditional Li⁺ cations can enter and leave the framework. In theseinstances additional Li⁺ cations can partially occupy the 16d octahedralsites normally occupied by the B-type cations. Under such circumstancesthese partially occupied octahedra can be considered to form part of theinterstitial space. Conversely, compounds can also be synthesized, inwhich part of the interstitial space defined by the 8a, 8b and 48ftetrahedral and 16c octahedral interstices of the Spinel structure canbe occupied by B-type cations, thereby rendering these particular sitesat least partially inaccessible to the mobile Li cations. The [B₂]X₄^(n−) framework structure can contain in certain instances a minorproportion, typically less than 10 atomic percent, of cations other thanthe mobile Li-type cations, or the A and B-type cations, within theframework structure or within the interstitial spaces of the frameworkstructure, and that could serve to stabilize the structure. For example,doped spinels of stoichiometry Li_(1+δ)Mn_(2−δ)O₄ where 0<δ≦0, 1, forexample, Li_(1.03)Mn_(1.97)O₄ in which δ=0, 03, and LiM_(δ/2)Mn_(2−δ)O₄where M=Mg or Zn and 0<δ≦0, 05, for example, LiMg_(0.025)Mn_(1.95)O₄,are more stable to cycling than the stoichiometric spinel LiMn₂O₄.

The compound of the anode may be a stoichiometric spinel selected fromthe group comprising Li₄Mn₅O₁₂, which can be written as(Li)_(8a)[Li_(0.33)Mn_(1.67)]_(16d)O₄ in ideal spinel notation;Li₄Ti₅O₁₂, which can be written as (Li)_(8a)[Li_(0.33)Ti_(1.67)]_(16d)O₄in ideal spinel notation; LiTi₂O₄ which can be written as(Li)_(8a)[Ti₂]_(16d)O₄ in ideal spinel notation; LiV₂O₄, which can bewritten as (Li)_(8a)[V₂]_(16d)O₄ in ideal spinel notation; and LiFe₅O₈,which can be written as (Fe)_(8a)[Fe_(1.5)Li_(0.5)]_(16d)O₄ in idealspinel notation.

Instead, the compound of the anode may be a defect spinel selected fromthe group comprising Li₂Mn₄O₉, which can be written as(Li_(0.89)□_(0.11))_(8a)[Mn_(1.78)□_(0.22)]_(16d)O₄ in spinel notation;and Li₂Ti₃O₇, which can be written as(Li_(0.85)□_(0.15))_(8a)[Ti_(1.71)Li_(0.29)]_(16d)O₄ in spinel notation.In defect spinels, the distribution of Li⁺ on the A and B sites can varyfrom compound to compound.

Instead, the compound of the anode may have a spinel-type structure,which can be a stoichiometric or defect spinel, with a mixture oftransition metal cations such as a lithium-iron-titanium oxide in whichthe lithium and iron cations are located on the A-sites, and lithium,iron and titanium cations on the B-sites.

In a preferred embodiment of the invention, the transition metalcations, Ti, V, Mn, Fe and Co, reside predominantly or completely on theB-sites of the spinel structure, while the Li cations residepredominantly or completely on the A-sites of the structure.

The lithium metal oxide compound of the cathode may also have aspinel-type framework structure. Thus, the framework structure of thelithium metal oxide compound of the cathode may then also have, as itsbasic structural unit, a unit of the formula [B₂]X₄ ^(n−) of an A[B₂]X₄spinel, as hereinbefore described, with the transition metal cations ofthe anode being more electropositive than those of the cathode.

In the compound of the cathode, A and B may be a metal cation of onetype, or a mixture of different metal cations. The compound of thecathode may be a stoichiometric or defect spinel compound, ashereinbefore described.

When the compound of the cathode has a spinel-type structure, it may beselected from the group having as its B-type cations Li, Mn, Co or Ni,or mixtures thereof, such as Li_(x)Mn₂O₄ where 0<x≦1 and Li_(x)CO₂O₄where 0<x≦2, optionally doped with additional metal cations to stabilizethe structure as hereinbefore described.

Instead, the compound of the cathode may have another structure type,for example a layered type structure such as that found within a systemdefined by a formula Li_(x)CO_(1−y)Ni_(y)O₂ where 0≦y≦1 and 0<x≦1.

In general, the anode compound will be selected from those spinelcompounds that offer a relatively low voltage vs pure lithium, typicallythose that offer 3V or less, while the cathode compound will be selectedfrom those spinel compounds that offer a relatively high voltage vs purelithium, typically those that offer between 4.5V and 3V. For example, aLi/Li_(4+x)Ti₅O₁₂ cell delivers on discharge at 100 μA/cm² (for 0<x<1)an average voltage of approximately 1.5V, while a Li/Li_(x)Mn₂O₄ celldelivers on discharge at 100 μA/cm² (for 0<x<1) an average voltage ofapproximately 4V. Therefore, a cell in accordance with the invention canhave Li_(4+x)Ti₅O₁₂ as an anode and Li_(x)Mn₂O₄ as a cathode, and willdeliver approximately 2.5V on discharge and which is approximately twicethe voltage of a nickel-cadmium cell. In another example, a Li/Li₂Mn₄O₉cell delivers a voltage of approximately 2.8V over most of thedischarge. Thus, a cell in accordance with the invention can have aLi_(2+x)Mn₄O₉ anode and Li_(x)Mn₂O₄ as cathode, and deliversapproximately 1.2V on discharge, which is the typical voltage of anickel-cadmium cell. It is convenient to load such cells in a dischargedstate, ie with the following configurations:Li₄Ti₅O₁₂/Electrolyte/LiMn₂O₄  (1)Li₂Mn₄O₉/Electrolyte/LiMn₂O₄  (2)

Although it is convenient to load such cells in a discharged state, thecells may also be loaded in the charged state, if so desired. In thisrespect, the anodes of the invention have lithiated spinel structuresand delithiated spinel structures that have the [B₂]X₄ spinel frameworkas defined hereinbefore.

In (1), Li⁺ ions are extracted from Li[Mn₂]O₄ during charge with aconcomitant oxidation of the manganese ions from an average valence of3.5 to higher values, and inserted into the Li₄Ti₅O₁₂ electrodestructure with a concomitant reduction of the titanium cations from theaverage valence state of +4 to lower values. During this process Li⁺ions are shuttled between the oxide structures without the formation ofany metallic lithium, the cell voltage being derived from changes in theoxidation state of the transition metal cations in the anode and cathodestructures.

The electrolyte may be a room temperature electrolyte such as LiClO₄,LiBF₄, or LiPF₆ dissolved in an appropriate organic salt such aspropylene carbonate, ethylene carbonate, dimethyl carbonate,dimethoxyethane, or appropriate mixtures thereof. Instead, however, itmay be any appropriate polymeric electrolyte such as polyethylene oxide(PEO)—LiClO₄, PEO—LiSO₃CF₃ and PEO—LiN(CF₃SO₂)₂, that operates at roomtemperature or at elevated temperature, eg at about 120° C.

The invention will now be described by way of non-limiting examples, andwith reference to the accompanying drawings in which:

FIG. 1 shows powder X-ray diffraction patterns of compounds suitable foruse as anode materials in rechargeable electrochemical cells accordingto the invention;

FIG. 2 shows powder X-ray diffraction patterns of compounds suitable foruse as cathode materials in rechargeable electrochemical cells accordingto the invention;

FIG. 3 shows a plot of voltage vs capacity for a known Li/Li₂Mn₄O₉ cell;

FIG. 4 shows a plot of voltage vs capacity for a known Li/Li₄Mn₅O₁₂cell;

FIG. 5 shows a plot of voltage vs capacity for a known Li/Li₄Ti₅O₁₂cell;

FIG. 6 shows a plot of voltage vs capacity for a known Li/LiFe₅O₈ cell;

FIG. 7 shows a plot of voltage vs capacity for a Li/Li—Fe—Ti oxide cell;

FIG. 8 shows a plot of voltage vs capacity for a known Li/LiMn₂O₄ cell;

FIG. 9 shows a plot of voltage vs capacity for a knownLi/Li_(1.03)Mn_(1.97)O₄ cell;

FIG. 10 shows a plot of voltage vs capacity for a known Li/LiCoO₂ cell;

FIG. 11 shows a plot of voltage vs capacity for the cell of Example 1and which is in accordance with the invention;

FIG. 12 shows a plot of voltage vs capacity for the cell of Example 2and which is in accordance with the invention;

FIG. 13 shows a plot of voltage vs capacity for the cell of Example 3and which is in accordance with the invention;

FIG. 14 shows a plot of voltage vs capacity for the cell of Example 4and which is in accordance with the invention;

FIG. 15 shows plots of voltage vs capacity for the cells of Examples 5and 6 and which are in accordance with the invention; and

FIG. 16 shows a cyclic voltammogram of the Li/Li—Fe—Ti oxide spinel cellof Example 7.

The following stoichiometric spinel and defect spinel compounds wereselected for use as anode materials in the examples followinghereinafter:

a) Li₂Mn₄O₉

b) Li₄Mn₅O₁₂

c) Li₄Ti₅O₁₂

d) LiFe₅O₈

e) Li—Fe—Ti oxide spinel in which Li:Fe:Ti=2:2:1

Powder X-ray diffraction patterns of these compounds are given in FIGS.1 a-e respectively.

The following spinel and non-spinel compounds were selected for use ascathode materials in the examples following hereinafter:

a) LiMn₂O₄ (spinel-type structure)

b) Li_(1.03)Mn_(1.97)O₄ (spinel-type structure)

c) LiCoO₂ (layered-type structure)

Powder X-ray diffraction patterns of these compounds are given in FIG. 2a-c respectively.

EXAMPLE 1

In view thereof that a Li/Li₂Mn₄O₉ cell delivers on discharge 150 mAh/gat an average voltage of approximately 2.8V, as indicated in FIG. 3, anda Li/LiMn₂O₄ cell delivers on discharge 120 mAh/g at an average voltageof approximately 3.8V, as indicated in FIG. 8, a cell in accordance withthe invention and having the configurationLi₂Mn₄O₉(anode)/Electrolyte/LiMn₂O₄(cathode) (2) was constructed.

The LiMn₂O₄ spinel compound of the cathode was synthesized by reactionof LiOH and γ-MnO₂ (chemically-prepared manganese dioxide, CMD) firstlyat 450° C. for 48 hours and thereafter at 750° C. for 48 hours. Thepowder X-ray diffraction pattern of this compound is shown in FIG. 2 a.

Li₂Mn₄O₉ was synthesized by reaction of LiOH and MnCO₃ at 345° C. for 32hours. The powder X-ray diffraction pattern of this compound is shown inFIG. 1 a. The pattern is predominantly characteristic of the Li₂Mn₄O₉defect spinel phase, but contains in addition a few very weak peaks, forexample at 42° 2θ and 53° 2θ, that are indicative of a very minorproportion of lithiated γ-MnO₂ phase.

A cell of the format Li₂Mn₄O₉/Electrolyte/LiMn₂O₄ (2) was thenconstructed. The electrolyte used was 1M LiClO₄ in propylene carbonate.The first 9 charge and 8 discharge cycles of the cell are shown in FIG.11. A current of 0.1 mA was employed for both charge and discharge. Thecell was cycled between upper and lower voltage limits of 1.5V and 0.45Vrespectively.

EXAMPLE 2

In view thereof that a Li/Li₄Mn₅O₁₂ cell delivers on discharge 150 mAh/gat an average voltage of approximately 2.7V, as indicated in FIG. 4, anda Li/Li_(1.03)Mn_(1.97)O₄ cell delivers on discharge 100 mAh/g at anaverage voltage of approximately 3.9V, as indicated in FIG. 9, a cell inaccordance with the invention and having the configurationLi₄Mn₅O₁₂/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (3) was constructed.

The Li_(1.03)Mn_(1.97)O₄ spinel compound of the cathode was synthesizedby the reaction of LiOH and γ-MnO₂ (chemically-prepared manganesedioxide, CMD) firstly at 450° C. for 48 hours and thereafter at 650° C.for 48 hours. The powder X-ray diffraction pattern of this compound isshown in FIG. 2 b.

Li₄Mn₅O₁₂ was synthesized by the reaction of Li₂CO₃ and MnCO₃ at 400° C.for 10 hours. The powder X-ray diffraction pattern of this compound isshown in FIG. 1 b. The pattern is predominantly characteristic of theLi₄Mn₅O₁₂ spinel phase.

A cell of the format Li₄Mn₅O₁₂/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (3) wasthen constructed. The electrolyte used was 1M LiClO₄ in propylenecarbonate. The first 5 charge/discharge cycles of the cell are shown inFIG. 12. A current of 0.1 mA was employed for both charge and discharge.The cell was cycled between upper and lower voltage limits of 1.6V and0.5V respectively.

EXAMPLE 3

In view thereof that a Li/Li₄Ti₅O₁₂ cell delivers on discharge 120 mAh/gat an average voltage of approximately 1.5V, as indicated in FIG. 5, anda Li/Li_(1.03)Mn_(1.97)O₄ cell delivers on discharge 100 mAh/g at anaverage voltage of approximately 3.9V, as indicated in FIG. 9, a cell inaccordance with the invention and having the configurationLi₄Ti₅O₁₂/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (4) was constructed.

The Li_(1.03)Mn_(1.97)O₄ spinel compound of the cathode was synthesizedas in Example 2.

Li₄Ti₅O₁₂ was synthesized by the reaction of Li₂CO₃ and TiO₂, using aLi/Ti atomic ratio of 0.87, at 500° C. for 12 hours and at 1000° C. for24 hours. A slight excess of lithium was used because of the volatilityof Li₂O at that temperature. The powder X-ray diffraction pattern ofthis compound is shown in FIG. 1 c. The pattern is predominantlycharacteristic of the Li₄Ti₅O₁₂ spinel phase.

A cell of the format Li₄Ti₅O₁₂/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (4) wasthen constructed. The electrolyte used was 1M LiClO₄ in propylenecarbonate. The first 7 charge/discharge cycles of the cell are shown inFIG. 13. A current of 0.1 mA was employed for both charge and discharge.The cell was cycled between upper and lower voltage limits of 2.8V and1.9V respectively.

EXAMPLE 4

In view thereof that a Li/Li₄Ti₅O₁₂ cell delivers on discharge 120mA·Hrs/g at an average voltage of approximately 1.5V, as indicated inFIG. 5, and a Li/LiCoO₂ cell delivers on discharge 140 mA·Hrs/g at anaverage voltage of approximately 3.9V, as indicated in FIG. 10, a cellin accordance with the invention and having the configurationLi₄Ti₅O₁₂/Electrolyte/LiCoO₂ (5) was constructed.

The LiCoO₂ spinel compound of the cathode was synthesized by thereaction of CoCO₃ and Li₂CO₃ firstly at 400° C. for 48 hours andthereafter at 900° C. for 48 hours. The powder X-ray diffraction patternof this compound is shown in FIG. 2 c.

Li₄Ti₅O₁₂ synthesized as in Example 3, was used for the anode in thisexample.

A cell of the format Li₄Ti₅O₁₂/Electrolyte/LiCoO₂ (5) was thenconstructed. The electrolyte used was 1M LiCoO₄ in propylene carbonate.The first 3 charge/discharge cycles of the cell are shown in FIG. 14. Acurrent of 0.1 mA was employed for both charge and discharge. The cellwas cycled between upper and lower voltage limits of 2.8V and 1.9Vrespectively.

EXAMPLE 5

In view thereof that a Li/LiFe₅O₈ cell delivers on discharge 100 mAh/gat an average voltage of approximately 1.0V, as indicated in FIG. 6, anda Li/Li_(1.05)Mn_(1.97)O₄ cell delivers on discharge 100 mAh/g at anaverage voltage of approximately 3.9V, as indicated in FIG. 9, a cell inaccordance with the invention and having the configurationLiFe₅O₈/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (6) was constructed.

The Li_(1.03)Mn_(1.97)O₄ spinel compound of the cathode was synthesizedas in Example 2.

LiFe₅O₈ was synthesized by reacting of Li₂CO₃ and α-Fe₂O₃ in a 1:5 molarratio at 900° C. for 24 hours. The powder X-ray diffraction pattern ofthis compound is shown in FIG. 1 d.

A cell of the format LiFe₅O₈/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (6) wasthen constructed. The electrolyte used was 1M LiClO₄ in propylenecarbonate. The first charge cycle of the cell is shown in FIG. 15 a. Acurrent of 0.1 mA was employed for both charge and discharge. The cellhad an upper voltage limit of 4.1V.

EXAMPLE 6

In view thereof that a Li/Li—Fe—Ti oxide spinel cell delivers ondischarge 80 mAh/g at an average voltage of approximately 0.6V, asindicated in FIG. 7, and a Li/Li_(1.03)Mn_(1.97)O₄ cell delivers ondischarge 100 mAh/g at an average voltage of approximately 3.9V, asindicated in FIG. 9, a cell in accordance with the invention and havingthe configuration Li—Fe—Ti oxide spinel/Electrolyte/Li_(1.03)Mn_(1.97)O₄(7) was constructed.

The Li_(1.03)Mn_(1.97)O₄ spinel compound of the cathode was synthesizedas in Example 2.

A Li—Fe—Ti oxide spinel was synthesized by the reaction of Li₂CO₃ andFe₂TiO₅, using a Li:Fe:Ti atomic ratio of 2:2:1, at 500° C. for 6 hoursand at 900° C. for 16 hours. The powder X-ray diffraction pattern ofthis compound is shown FIG. 1 e. The pattern is predominantlycharacteristic of a spinel-type phase.

A cell of the format Li—Fe—Ti oxidespinel/Electrolyte/Li_(1.03)Mn_(1.97)O₄ (7) was then constructed. Theelectrolyte used was 1M LiClO₄ in propylene carbonate. The first chargecycle of the cell is shown in FIG. 15 b. A current of 0.1 mA wasemployed for both charge and discharge. The cell had an upper voltagelimit of 4.4V.

EXAMPLE 7

A Li—Fe—Ti oxide spinel was synthesized by the reaction Li₂CO₃ andFe₂TiO₃ using a Li:Fe:Ti atomic ratio of 1:2:1 at 500° C. for 6 hours,and thereafter at 900° C. for 16 hours. A cyclic voltammogram of aLi/Li—Fe—Ti oxide spinel cell with an electrolyte of 1M LiCO₄ inpropylene carbonate is shown in FIG. 16. It shows the rechargeablecharacteristics of the Li—Fe—Ti oxide spinel electrode, and inparticular, the rechargeability of the Li insertion/extraction reactionthat occurs at approximately 1.5V versus lithium.

Examples 5, 6 and 7 show, in particular, the potential of usingspinel-type oxides containing iron as anodes because they provide a lowvoltage against lithium. Furthermore, the experimental data provided inthe examples demonstrate the ability of transition metal oxides toprovide an electrochemical couple for ‘rocking chair’ rechargeablelithium cells in which lithium ions are transported between the twotransition metal oxide electrodes, the anode of which has a spinel-typestructure, and which uses a liquid or polymeric electrolyte containingLi⁺ ions. The electrochemical cells of the invention thus contain nometallic lithium anode, and are therefore inherently safer than lithiumcells containing metallic lithium anodes and, indeed, lithium-carbonanodes. In particular, such cells have an added advantage of providing amore constant operating voltage than cells with carbon anodes. Althoughthe cells of the invention are designed primarily for the use asrechargeable cells, they can also, as indicated hereinbefore, beutilized as primary cells, if desired.

Although the principles of this invention have been demonstrated by useof lithium-metal oxide compounds, the compounds of the electrodes,instead of being oxides, can be sulphides.

1. An electrochemical cell comprising: as at least part of an anode, a lithium transition metal oxide compound which has a [B₂]X₄ ^(n−) spinel-type framework structure of an A[B₂]X₄ stoichiometric spinel or defect spinel, wherein A comprises Li, B comprises Li and Ti, X is oxygen (O), and n− refers to the overall charge of the structural unit [B₂]X₄ ^(n−) of the framework structure, and the transition metal cation of which in the fully discharged state of the cell has a mean oxidation state of +4 for Ti; as at least part of a cathode, a compound with a structure type other than a lithium-metal-oxide compound; and an electrically insulative, lithium containing, liquid or polymeric, ionically conductive electrolyte between the anode and the cathode, such that, on discharging the cell, lithium ions are extracted from the spinel-type framework structure of the anode, with the oxidation state of the metal ions of the anode thereby increasing, while a concomitant insertion of lithium ions into the compound of the cathode takes place, with the oxidation state of the metal ions of the cathode decreasing correspondingly.
 2. The electrochemical cell of claim 1, wherein, in the compound of the anode, the [B₂]X₄ ^(n−) framework structure contains, within the framework structure or within interstitial spaces present in the framework structure, additional metal cations to the lithium ions and the other A and B cations, with the additional metal cations being present in an amount less than 10 atomic percent.
 3. The electrochemical cell of claim 1, wherein the cathode comprises a lithium metal sulfide compound.
 4. The electrochemical cell of claim 1, wherein the electrolyte is a room temperature electrolyte selected from the group consisting of LiClO₄, LiBF₄ and LiPF₆ dissolved in an organic solvent selected from the group consisting of propylene carbonate, ethylene carbonate, dimethyl carbonate, dimethoxyethane and mixtures thereof.
 5. The electrochemical cell of claim 1, wherein the electrolyte is a polymeric electrolyte selected from the group consisting of polyethylene oxide (PEO)—LiClO₄, PEO—LiSO₃CF₃, and PEO—LiN(CF₃SO₂)₂. 